Answer
$\Delta S_{univ}=162\,J/K$, the reaction is spontaneous.
Work Step by Step
For a spontaneous process, $\Delta S_{univ}$ is positive.
$\Delta S_{univ}=\Delta S_{sys}+\Delta S_{surr}$
$\Delta S_{surr}=\frac{-\Delta H_{sys}}{T}=\frac{-(-95\,kJ)}{298\,K}=\frac{95\times10^{3}\,J}{298\,K}=319\,J/K$
$\Delta S_{sys}=-157\,J/K$
Therefore,
$\Delta S_{univ}=(-157\,J/K)+(319\,J/K)=162\,J/K$
As $\Delta S_{univ}$ is positive, the reaction is spontaneous.
